Which of the following equations represents standard heat of formation of ${C H}_{4}$ ?

C_{(d i a m o n d)} + 2 H_{2 (g)} \to {C H}_{4 (g)}

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C_{(g r a p h i t e)} + 2 H_{2 (g)} \to {C H}_{4 (g)}

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C_{(d i a m o n d)} + 4 H_{2 (g)} \to {C H}_{4 (g)}

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C_{(g r a p h i t e)} + 4 H_{2 (g)} \to {C H}_{4 (g)}

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Solution

The correct option is B $C_{(g r a p h i t e)} + 2 H_{2 (g)} \to {C H}_{4 (g)}$
The standard enthalpy of formation or standard heat of formation of a compound is the change of enthalpy during the formation of 1 mole of the substance from its constituent elements, with all substances in their standard states.

We know that the standard state for carbon is its graphite form, for hydrogen, its gaseous form. Also, it is necessary for the equation to be balanced.

Since, option (B) meets all the above requirements,

Hence, option (B) is the correct answer.

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Similar questions

C (d i a m o n d) + 2 H_{2} (g) ⟶ C H_{4} (g); Δ H_{1}

C (g) + 4 H (g) ⟶ C H_{4} (g); Δ H_{2}

C_{(g r a p h i t e)} + 2 H_{2 (g)} \to C H_{4 (g)}

Δ o f C H_{4} = - 74.81 K J m o l^{- 1}

Δ S^{\circ} o f C_{g r a p h i t e}, H_{2 (g)} a n d C H_{4 (g)} a r e 5.70 K^{- 1} m o l^{- 1}, a n d 186.3 J K^{- 1} m o l^{- 1}

C (d i a m o n d) + 2 H_{2} (g) ⟶ C H_{4} (g)

Δ H

Δ U

C_{(g r a p h i t e)} + O_{2} (g) \to C O_{2} (g); Δ_{r} H^{o} = - 393.5 k J m o l^{- 1}

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l); Δ_{r} H^{o} = - 285.8 k J m o l^{- 1}

C O_{2} (g) + 2 H_{2} O (l) \to C H_{4} (g) + 2 O_{2} (g); Δ_{r} H^{o} = + 890.3 k J m o l^{- 1}

Δ_{r} H^{o}

298 K

C_{(g r a p h i t e)} + 2 H_{2} (g) \to C H_{4} (g)

C H_{4}

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